1. CHEMISTRY SEMESTER 2 FINAL EXAM REVIEW QUESTIONS..

2. Chapter 6
1. A chemical bond results from the mutual attraction of the nuclei for
A. electrons.
B. neutrons.
C. protons.
D. dipoles.

3. Chapter 6
1. A chemical bond results from the mutual attraction of the nuclei for
A. electrons.
B. neutrons.
C. protons.
D. dipoles.

4. 2. A polar covalent bond is likely to form between two atoms that
Chapter 6
2. A polar covalent bond is likely to form between two atoms that
A. are similar in electronegativity.
B. are of similar size.
C. differ in electronegativity.
D. have the same number of electrons.

5. 2. A polar covalent bond is likely to form between two atoms that
Chapter 6
2. A polar covalent bond is likely to form between two atoms that
A. are similar in electronegativity.
B. are of similar size.
C. differ in electronegativity.
D. have the same number of electrons.

6. Chapter 6
3. The Lewis structure of HCN contains A. one double bond and one single bond. B. one triple bond and one single bond. C. two single bonds. D. two double bonds.

7. Chapter 6
3. The Lewis structure of HCN contains A. one double bond and one single bond. B. one triple bond and one single bond. C. two single bonds. D. two double bonds.

8. 4. According to VSEPR theory, the molecular geometry for is
Chapter 6
4. According to VSEPR theory, the molecular geometry for is
A. tetrahedral.
B. trigonal-pyramidal.
C. bent or angular.
D. None of the above

9. 4. According to VSEPR theory, the molecular geometry for is
Chapter 6
4. According to VSEPR theory, the molecular geometry for is
A. tetrahedral.
B. trigonal-pyramidal.
C. bent or angular.
D. None of the above

10. Chapter 6
5. Which molecule contains a double bond? A. COCl2 B. C2H6 C. CF4 D. SF2

11. Chapter 6
5. Which molecule contains a double bond? A. COCl2 B. C2H6 C. CF4 D. SF2

12. 6. Which molecule is polar? A. CCl4 B. CO2 C. SO3 D. none of these
Chapter 6
6. Which molecule is polar?
A. CCl4
B. CO2
C. SO3
D. none of these

13. 6. Which molecule is polar? A. CCl4 B. CO2 C. SO3 D. none of these
Chapter 6
6. Which molecule is polar?
A. CCl4
B. CO2
C. SO3
D. none of these

14. Chapter 6
7. What is the hybridization of the carbon atoms in CH4? A. sp B. sp2 C. sp3 D. The carbon atoms do not hybridize in C2H2.

15. Chapter 6
7. What is the hybridization of the carbon atoms in CH4? A. sp B. sp2 C. sp3 D. The carbon atoms do not hybridize in C2H2.

16. Chapter 6
8. Which of the following compounds is predicted to have the highest boiling point?
A. HCl
B. CH3COOH (Note: the two oxygen atoms bond to the carbon)
C. Cl2
D. SO2

17. Chapter 6
8. Which of the following compounds is predicted to have the highest boiling point?
A. HCl
B. CH3COOH (Note: the two oxygen atoms bond to the carbon)
C. Cl2
D. SO2

18. Chapter 6
9. An unknown substance is an excellent electrical conductor in the solid state and is malleable. What type of chemical bonding does this substance exhibit? A. ionic bonding B. molecular bonding C. metallic bonding D. cannot determine from the information given

19. Chapter 6
9. An unknown substance is an excellent electrical conductor in the solid state and is malleable. What type of chemical bonding does this substance exhibit? A. ionic bonding B. molecular bonding C. metallic bonding D. cannot determine from the information given

20. 10. What does the hybridization model help explain?
Chapter 6
10. What does the hybridization model help explain?
a. Explains how the orbitals of an atom become rearranged when the atom forms covalent bonds.
b. Geometry of molecule
c. Rates of reactions
d. Polarity of a bond

21. 10. What does the hybridization model help explain?
Chapter 6
10. What does the hybridization model help explain?
a. Explains how the orbitals of an atom become rearranged when the atom forms covalent bonds.
b. Geometry of molecule
c. Rates of reactions
d. Polarity of a bond

22. Chapter 6
12. Naphthalene, C10H8, is a nonpolar molecule and has a boiling point of 218°C. Acetic acid, CH3CO2H, is a polar molecule and has a boiling point of 118°C. Which substance has the stronger intermolecular forces? Briefly explain your answer.

23. Chapter 6
12. Naphthalene, C10H8, is a nonpolar molecule and has a boiling point of 218°C. Acetic acid, CH3CO2H, is a polar molecule and has a boiling point of 118°C. Which substance has the stronger intermolecular forces? Briefly explain your answer. Answer: Naphthalene has the stronger intermolecular forces even though it is nonpolar, because its boiling point is higher than that of acetic acid. Boiling point is directly correlated to strength of intermolecular forces; the stronger the intermolecular forces, the more energy needed to break all the intermolecular forces, and therefore the higher the boiling point. Naphthalene is so large that its dispersion forces are greater than the sum of the dispersion forces and hydrogen bonding in acetic acid.

24. A. sodium carbonate B. sodium sulfate C. sodium sulfite
Chapter 7
1. Which of the following compounds does not contain a polyatomic ion?
A. sodium carbonate
B. sodium sulfate
C. sodium sulfite
D. sodium sulfide

25. A. sodium carbonate B. sodium sulfate C. sodium sulfite
Chapter 7
1. Which of the following compounds does not contain a polyatomic ion?
A. sodium carbonate
B. sodium sulfate
C. sodium sulfite
D. sodium sulfide

26. 2. The correct formula for ammonium phosphate is
Chapter 7
2. The correct formula for ammonium phosphate is
A. (NH4)3PO4.
B. (NH4)2PO4.
C. NH4PO4.
D. NH4(PO4)2.

27. 2. The correct formula for ammonium phosphate is
Chapter 7
2. The correct formula for ammonium phosphate is
A. (NH4)3PO4.
B. (NH4)2PO4.
C. NH4PO4.
D. NH4(PO4)2.

28. A. write the anion’s formula first.
Chapter 7
When writing the formula for a compound that contains a polyatomic ion,
A. write the anion’s formula first.
B. use superscripts to show the number of polyatomic ions present.
C. use parentheses if the number of polyatomic ions is greater than 1.
D. always place the polyatomic ion in parentheses.

29. A. write the anion’s formula first.
Chapter 7
When writing the formula for a compound that contains a polyatomic ion,
A. write the anion’s formula first.
B. use superscripts to show the number of polyatomic ions present.
C. use parentheses if the number of polyatomic ions is greater than 1.
D. always place the polyatomic ion in parentheses.

30. The correct name for NH4CH3COO or NH4CH2COOH is
Chapter 7
The correct name for NH4CH3COO or NH4CH2COOH is
A. ammonium carbonate.
B. ammonium hydroxide.
C. ammonium acetate.
D. ammonium nitrate.

31. The correct name for NH4CH3COO or NH4CH2COOH is
Chapter 7
The correct name for NH4CH3COO or NH4CH2COOH is
A. ammonium carbonate.
B. ammonium hydroxide.
C. ammonium acetate.
D. ammonium nitrate.

32. Which of the following is the correct formula for iron(III) sulfate?
Chapter 7
Which of the following is the correct formula for iron(III) sulfate?
A. Fe3SO4
B. Fe3(SO4)2
C. Fe2(SO4)3
D. 3FeSO4

33. Which of the following is the correct formula for iron(III) sulfate?
Chapter 7
Which of the following is the correct formula for iron(III) sulfate?
A. Fe3SO4
B. Fe3(SO4)2
C. Fe2(SO4)3
D. 3FeSO4

34. Chapter 7
The molecular formula for acetylene is C2H2. The molecular formula for benzene is C6H6. The empirical formula for both is
A. CH.
B. C2H2.
C. C6H6.
D. (CH)2.

35. Chapter 7
The molecular formula for acetylene is C2H2. The molecular formula for benzene is C6H6. The empirical formula for both is
A. CH.
B. C2H2.
C. C6H6.
D. (CH)2.

36. Which of the following shows the percentage composition of H2SO4?
Chapter 7
Which of the following shows the percentage composition of H2SO4?
A. 2.5% H, 39.1% S, 58.5% O
B. 2.1% H, 32.7% S, 65.2% O
C. 28.6% H, 14.3% S, 57.1% O
D. 33.3% H, 16.7% S, 50% O

37. Which of the following shows the percentage composition of H2SO4?
Chapter 7
Which of the following shows the percentage composition of H2SO4?
A. 2.5% H, 39.1% S, 58.5% O
B. 2.1% H, 32.7% S, 65.2% O
C. 28.6% H, 14.3% S, 57.1% O
D. 33.3% H, 16.7% S, 50% O

38. Which of the following compounds has the highest percentage of oxygen?
Chapter 7
Which of the following compounds has the highest percentage of oxygen?
A. CH4O
B. CO2
C. H2O
D. Na2CO3

39. Which of the following compounds has the highest percentage of oxygen?
Chapter 7
Which of the following compounds has the highest percentage of oxygen?
A. CH4O
B. CO2
C. H2O
D. Na2CO3

40. Chapter 7
The empirical formula for a compound that is 1.2% H, 42.0% Cl, and 56.8% O is
A. HClO.
B. HClO2.
C. HClO3.
D. HClO4.

41. Chapter 7
The empirical formula for a compound that is 1.2% H, 42.0% Cl, and 56.8% O is
A. HClO.
B. HClO2.
C. HClO3.
D. HClO4.

42. Chapter 7
When a new substance is synthesized or is discovered experimentally, the substance is analyzed quantitatively. What information is obtained from this typical analysis, and how is this information used?

43. Chapter 7
When a new substance is synthesized or is discovered experimentally, the substance is analyzed quantitatively. What information is obtained from this typical analysis, and how is this information used?
Answer: The percentage composition is obtained and used to determine the substance’s empirical formula.

44. Chapter 7
An oxide of selenium is 28.8% O. Find the empirical formula. Assuming that the empirical formula is also the molecular formula, name the oxide.

45. Answer: SeO2; selenium dioxide
Chapter 7
An oxide of selenium is 28.8% O. Find the empirical formula. Assuming that the empirical formula is also the molecular formula, name the oxide.
Answer: SeO2; selenium dioxide

46. Chapter 7
What is an empirical formula, and how does it differ from a molecular formula?

47. Chapter 7
What is an empirical formula, and how does it differ from a molecular formula?
Answer: The empirical formula is the simplest whole-number ratio of the atoms in a chemical formula. The molecular formula is the actual number of atoms of each element in a chemical formula. The two formulas differ by an integer factor.

48. A. always more than the total mass of the products.
Chapter 8
According to the law of conservation of mass, the total mass of the reacting substances is
A. always more than the total mass of the products.
B. always less than the total mass of the products.
C. sometimes more and sometimes less than the total mass of the products.
D. always equal to the total mass of the products.

49. A. always more than the total mass of the products.
Chapter 8
According to the law of conservation of mass, the total mass of the reacting substances is
A. always more than the total mass of the products.
B. always less than the total mass of the products.
C. sometimes more and sometimes less than the total mass of the products.
D. always equal to the total mass of the products.

50. To balance a chemical equation, you may adjust the A. coefficients.
Chapter 8
To balance a chemical equation, you may adjust the
A. coefficients.
B. subscripts.
C. formulas of the products.
D. either the coefficients or the subscripts.

51. To balance a chemical equation, you may adjust the A. coefficients.
Chapter 8
To balance a chemical equation, you may adjust the
A. coefficients.
B. subscripts.
C. formulas of the products.
D. either the coefficients or the subscripts.

52. Chapter 8
Which is the correct chemical equation for the following formula equation:
(NH4)2S NH3 + H2S?
A. 2(NH4)2S NH3 + H2S2
B. 2(NH4)2S NH3 + H2S
C. (NH4)2S 2NH3 + H2S
D. None of the above

53. Chapter 8
Which is the correct chemical equation for the following formula equation:
(NH4)2S NH3 + H2S?
A. 2(NH4)2S NH3 + H2S2
B. 2(NH4)2S NH3 + H2S
C. (NH4)2S 2NH3 + H2S
D. None of the above

54. Select the missing reactant for the following combustion reaction:
Chapter 8
Select the missing reactant for the following combustion reaction:
2______ + 15O CO2 + 6H2O.
A. C14H12
B. C14H12O4
C. C7H6
D. C7H6O2

55. Select the missing reactant for the following combustion reaction:
Chapter 8
Select the missing reactant for the following combustion reaction:
2_____ + 15O CO2 + 6H2O.
A. C14H12
B. C14H12O4
C. C7H6
D. C7H6O2

56. Chapter 8
Which of the following statements is true about the reaction
2F2 + 2H2O HF + O2?
A. Two grams of O2 are produced when 2 g F2 reacts
with 2 g H2O.
B. Two moles of HF are produced when 1 mol F2
reacts with 1 mol H2O.
C. For every 2 mol O2 produced, 6 mol HF are produced.
D. For every 1 mol H2O that reacts, 2 mol O2 are produced.

57. Chapter 8
Which of the following statements is true about the reaction
2F2 + 2H2O HF + O2?
A. Two grams of O2 are produced when 2 g F2 reacts
with 2 g H2O.
B. Two moles of HF are produced when 1 mol F2
reacts with 1 mol H2O.
C. For every 2 mol O2 produced, 6 mol HF are produced.
D. For every 1 mol H2O that reacts, 2 mol O2 are produced.

58. Chapter 8
Short Answer
A precipitation of iron(III) hydroxide is produced by reacting an aqueous solution of iron(III) chloride with an aqueous solution of sodium hydroxide. Write a balanced chemical equation.

59. FeCl3(aq) + 3NaOH(aq) Fe(OH)3(s) + 3NaCl(aq)
Chapter 8
Short Answer
A precipitation of iron(III) hydroxide is produced by reacting an aqueous solution of iron(III) chloride with an aqueous solution of sodium hydroxide. Write a balanced chemical equation.
Answer:
FeCl3(aq) + 3NaOH(aq) Fe(OH)3(s) + 3NaCl(aq)

60. In stoichiometry, chemists are mainly concerned with
A. the types of bonds found in compounds.
B. mass relationships in chemical reactions.
C. energy changes occurring in chemical reactions.
D. the speed with which chemical reactions occur.

61. In stoichiometry, chemists are mainly concerned with
A. the types of bonds found in compounds.
B. mass relationships in chemical reactions.
C. energy changes occurring in chemical reactions.
D. the speed with which chemical reactions occur.

62. Assume ideal stoichiometry in the reaction CH4 + 2O2 → CO2 + 2H2O
Assume ideal stoichiometry in the reaction CH4 + 2O2 → CO2 + 2H2O. If you know the mass of CH4, you can calculate
A. only the mass of CO2 produced.
B. only the mass of O2 reacting.
C. only the mass of CO2 + H2O produced.
D. the mass of O2 reacting and CO2 + H2O produced.

63. Assume ideal stoichiometry in the reaction CH4 + 2O2 → CO2 + 2H2O
Assume ideal stoichiometry in the reaction CH4 + 2O2 → CO2 + 2H2O. If you know the mass of CH4, you can calculate
A. only the mass of CO2 produced.
B. only the mass of O2 reacting.
C. only the mass of CO2 + H2O produced.
D. the mass of O2 reacting and CO2 + H2O produced.

64. Which mole ratio for the equation 6Li + N2 → 2Li3N is incorrect?
A C.
B D.
2 mol Li3N
1 mol N2
6 mol Li
2 mol N2
2 mol Li3N
6 mol Li
1 mol N2
6 mol Li

65. Which mole ratio for the equation 6Li + N2 → 2Li3N is incorrect?
A C.
B D.
2 mol Li3N
1 mol N2
6 mol Li
2 mol N2
2 mol Li3N
6 mol Li
1 mol N2
6 mol Li

66. For the reaction below, how many moles of N2 are required to produce 18 mol NH3?
N2 + 3H2 → 2NH3
A. 4.5
B. 9.0
C. 18
D. 36

67. For the reaction below, how many moles of N2 are required to produce 18 mol NH3?
N2 + 3H2 → 2NH3
A. 4.5
B. 9.0
C. 18
D. 36

68. What mass of NaCl can be produced by the reaction of 0.75 mol Cl2?
2Na + Cl2 → 2NaCl
A g
B. 1.5 g
C. 44 g
D. 88 g

69. What mass of NaCl can be produced by the reaction of 0.75 mol Cl2?
2Na + Cl2 → 2NaCl
A g
B. 1.5 g
C. 44 g
D. 88 g

70. What mass of CO2 can be produced from 25
What mass of CO2 can be produced from g CaCO3 given the decomposition reaction
CaCO3 → CaO + CO2
A g
B g
C g
D g

71. What mass of CO2 can be produced from 25
What mass of CO2 can be produced from g CaCO3 given the decomposition reaction
CaCO3 → CaO + CO2
A g
B g
C g
D g

72. A. excess reactant. B. primary reactant. C. limiting reactant.
If a chemical reaction involving substances A and B stops when B is completely used up, then B is referred to as the
A. excess reactant.
B. primary reactant.
C. limiting reactant.
D. primary product.

73. A. excess reactant. B. primary reactant. C. limiting reactant.
If a chemical reaction involving substances A and B stops when B is completely used up, then B is referred to as the
A. excess reactant.
B. primary reactant.
C. limiting reactant.
D. primary product.

74. If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
A. percentage yield.
B. mole ratio.
C. theoretical yield.
D. actual yield.

75. If a chemist calculates the maximum amount of product that could be obtained in a chemical reaction, he or she is calculating the
A. percentage yield.
B. mole ratio.
C. theoretical yield.
D. actual yield.

76. What is the maximum number of moles of AlCl3 that can be produced from 5.0 mol Al and 6.0 mol Cl2?
2Al + 3Cl2 → 2AlCl3
A. 2.0 mol AlCl3
B. 4.0 mol AlCl3
C. 5.0 mol AlCl3
D. 6.0 mol AlCl3

77. What is the maximum number of moles of AlCl3 that can be produced from 5.0 mol Al and 6.0 mol Cl2?
2Al + 3Cl2 → 2AlCl3
A. 2.0 mol AlCl3
B. 4.0 mol AlCl3
C. 5.0 mol AlCl3
D. 6.0 mol AlCl3

78. Short Answer
Why is a balanced equation necessary to solve a mass-mass stoichiometry problem?

79. Short Answer
Why is a balanced equation necessary to solve a mass-mass stoichiometry problem?
Answer: The coefficients of the balanced equation are needed for the mole-mole ratio that is necessary to solve stoichiometric problems involving two different substances.

80. Short Answer
What data are necessary to calculate the percentage yield of a reaction?

81. Short Answer
What data are necessary to calculate the percentage yield of a reaction?
Answer: the theoretical yield and the actual yield of the product

82. Extended Response
A student makes a compound in the laboratory and reports an actual yield of 120%. Is this result possible? Assuming that all masses were measured correctly, give an explanation.

83. Extended Response
A student makes a compound in the laboratory and reports an actual yield of 120%. Is this result possible? Assuming that all masses were measured correctly, give an explanation.
Answer: The product was impure, so the mass contained the product and other substances. For example, if NaCl is made from HCl and NaOH but is not dried, the mass of NaCl can include water, which would result in a yield greater than 100%.

84. Extended Response
Benzene, C6H6, is reacted with bromine, Br2, to produce bromobenzene, C6H5Br, and hydrogen bromide, HBr, as shown below. When 40.0 g of benzene are reacted with 95.0 g of bromine, 65.0 g of bromobenzene is produced.
C6H6 + Br2 → C6H5Br + HBr
a. Which compound is the limiting reactant?
b. What is the theoretical yield of bromobenzene?
c. What is the reactant in excess, and how much remains after the reaction is completed?
d. What is the percentage yield?

85. Extended Response
Benzene, C6H6, is reacted with bromine, Br2, to produce bromobenzene, C6H5Br, and hydrogen bromide, HBr, as shown below. When 40.0 g of benzene are reacted with g of bromine, 65.0 g of bromobenzene is produced.
C6H6 + Br2 → C6H5Br + HBr
a. Which compound is the limiting reactant? benzene
b. What is the theoretical yield of bromobenzene? g
c. What is the reactant in excess, and how much remains after the reaction is completed? bromine, 13.2 g
d. What is the percentage yield? 80.8%

86. Chapter 11
Pressure can be measured in
A. grams.
B. meters.
C. mmHg.
D. liters.

87. Chapter 11
Pressure can be measured in
A. grams.
B. meters.
C. mmHg.
D. liters.

88. Chapter 11
A sample of oxygen gas has a volume of 150 mL when its pressure is atm. If the pressure is increased to atm and the temperature remains constant, what will the new volume be?
A. 140 mL
B. 160 mL
C. 200 mL
D. 240 mL

89. Chapter 11
A sample of oxygen gas has a volume of 150 mL when its pressure is atm. If the pressure is increased to atm and the temperature remains constant, what will the new volume be?
A. 140 mL
B. 160 mL
C. 200 mL
D. 240 mL

90. A sample of gas in a closed container at a temperature of 100
A sample of gas in a closed container at a temperature of 100.0°C and 3.0 atm is heated to 300.0°C. What is the pressure of the gas at the higher temperature?
A. 35 atm
B. 4.6 atm
C. 59 atm
D. 9.0 atm

91. A sample of gas in a closed container at a temperature of 100
A sample of gas in a closed container at a temperature of 100.0°C and 3.0 atm is heated to 300.0°C. What is the pressure of the gas at the higher temperature?
A. 35 atm
B. 4.6 atm
C. 59 atm
D. 9.0 atm

92. Avogadro’s law states that
Chapter 11
Avogadro’s law states that
A. equal numbers of moles of gases at the same conditions occupy equal volumes, regardless of the identity of the gases.
B. at constant pressure, gas volume is directly proportional to absolute temperature.
C. the volume of a gas is inversely proportional to its amount in moles.
D. at constant temperature, gas volume is inversely proportional to pressure.

93. Avogadro’s law states that
Chapter 11
Avogadro’s law states that
A. equal numbers of moles of gases at the same conditions occupy equal volumes, regardless of the identity of the gases.
B. at constant pressure, gas volume is directly proportional to absolute temperature.
C. the volume of a gas is inversely proportional to its amount in moles.
D. at constant temperature, gas volume is inversely proportional to pressure.

94. Chapter 11
Short Answer
Give a molecular explanation for the observation that the pressure of a gas increases when the gas volume is decreased.

95. Chapter 11
Short Answer
Give a molecular explanation for the observation that the pressure of a gas increases when the gas volume is decreased.
Answer: The molecules are closer together, so they strike the walls of the container more often.

96. Chapter 12
Water is an excellent solvent because
A. it is a covalent compound.
B. it is a nonconductor of electricity.
C. its molecules are quite polar.
D. it is a clear, colorless liquid.

97. Chapter 12
Water is an excellent solvent because
A. it is a covalent compound.
B. it is a nonconductor of electricity.
C. its molecules are quite polar.
D. it is a clear, colorless liquid.

98. Chapter 12
Two liquids are likely to be immiscible if
A. both have polar molecules.
B. both have nonpolar molecules.
C. one is polar and the other is nonpolar.
D. one is water and the other is methyl alcohol, CH3OH.

99. Chapter 12
Two liquids are likely to be immiscible if
A. both have polar molecules.
B. both have nonpolar molecules.
C. one is polar and the other is nonpolar.
D. one is water and the other is methyl alcohol, CH3OH.

100. Chapter 12
Which of the following types of compounds is most likely to be a strong electrolyte?
A. a polar compound
B. a nonpolar compound
C. a covalent compound
D. an ionic compound

101. Chapter 12
Which of the following types of compounds is most likely to be a strong electrolyte?
A. a polar compound
B. a nonpolar compound
C. a covalent compound
D. an ionic compound

102. Chapter 12
Molarity is expressed in units of
A. moles of solute per liter of solution.
B. liters of solution per mole of solute.
C. moles of solute per liter of solvent.
D. liters of solvent per mole of solute.

103. Chapter 12
Molarity is expressed in units of
A. moles of solute per liter of solution.
B. liters of solution per mole of solute.
C. moles of solute per liter of solvent.
D. liters of solvent per mole of solute.

104. Chapter 12
Molarity is expressed in units of
A. moles of solute per liter of solution.
B. liters of solution per mole of solute.
C. moles of solute per liter of solvent.
D. liters of solvent per mole of solute.

105. What mass of NaOH is contained in 2.5 L of a 0.010 M solution?
Chapter 12
What mass of NaOH is contained in 2.5 L of a M solution?
A g
B. 1.0 g
C. 2.5 g
D g

106. What mass of NaOH is contained in 2.5 L of a 0.010 M solution?
Chapter 12
What mass of NaOH is contained in 2.5 L of a M solution?
A g
B. 1.0 g
C. 2.5 g
D g

107. Chapter 12
Which one of the following statements is false?
A. Gases are generally more soluble in water under high pressures than under low pressures.
B. As temperature increases, the solubilities of some solids in water increase and the solubilities of other solids in water decrease.
C. Water dissolves many ionic solutes because of its ability to hydrate ions in solution.
D. Many solids dissolve more quickly in a cold solvent than in a warm solvent.

108. Chapter 12
Which one of the following statements is false?
A. Gases are generally more soluble in water under high pressures than under low pressures.
B. As temperature increases, the solubilities of some solids in water increase and the solubilities of other solids in water decrease.
C. Water dissolves many ionic solutes because of its ability to hydrate ions in solution.
D. Many solids dissolve more quickly in a cold solvent than in a warm solvent.

109. Chapter 12
Extended Response
Explain why oil and water do not mix.

110. Chapter 12 Extended Response Explain why oil and water do not mix.
Answer: Water is polar, and oil is nonpolar. When the two are combined, the strong hydrogen bonding between water molecules squeezes out the oil droplets, forming separate layers.

111. Chapter 12 Extended Response
Write a set of instructions on how to prepare a solution that is M KBr, using solid KBr (molar mass 119 g/mol) as the solute. Your instructions should include a list of all materials and equipment needed.

112. Chapter 12 Extended Response
Write a set of instructions on how to prepare a solution that is M KBr, using solid KBr (molar mass 119 g/mol) as the solute. Your instructions should include a list of all materials and equipment needed.
Answer: Your answer should summarize the steps using 11.9 g of KBr in a 1.00 L volumetric flask (or values proportional to these).

113. Acetic acid is a weak electrolyte because it
Chapter 13
Acetic acid is a weak electrolyte because it
A. is miscible with water.
B. forms hydronium and hydroxide ions in
aqueous solution.
C. lowers the freezing point of water.
D. ionizes only slightly in aqueous solution.

114. Acetic acid is a weak electrolyte because it
Chapter 13
Acetic acid is a weak electrolyte because it
A. is miscible with water.
B. forms hydronium and hydroxide ions in
aqueous solution.
C. lowers the freezing point of water.
D. ionizes only slightly in aqueous solution.

115. Chapter 14
Which of the following is not a characteristic of
an acid?
A. An acid changes the color of an indicator.
B. An acid has a bitter taste.
C. An acid ionizes in water.
D. An acid produces hydronium ions in water.

116. Chapter 14
Which of the following is not a characteristic of
an acid?
A. An acid changes the color of an indicator.
B. An acid has a bitter taste.
C. An acid ionizes in water.
D. An acid produces hydronium ions in water.

117. Chapter 14
When an acid reacts with an active metal,
A. the hydronium ion concentration increases.
B. the metal forms anions.
C. hydrogen gas is produced.
D. carbon dioxide gas is produced.

118. Chapter 14
When an acid reacts with an active metal,
A. the hydronium ion concentration increases.
B. the metal forms anions.
C. hydrogen gas is produced.
D. carbon dioxide gas is produced.

119. Chapter 14
Which of the following is a Brønsted-Lowry base?
A. an electron pair donor
B. an electron pair acceptor
C. a proton donor
D. a proton acceptor

120. Chapter 14
Which of the following is a Brønsted-Lowry base?
A. an electron pair donor
B. an electron pair acceptor
C. a proton donor
D. a proton acceptor

121. Chapter 14
What is the formula for acetic acid?
A. CH3COOH
B. HNO3
C. HClO4
D. HCN

122. Chapter 14
What is the formula for acetic acid?
A. CH3COOH
B. HNO3
C. HClO4
D. HCN

123. Chapter 14
Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.
A. calcium sulfate
B. calcium hydroxide
C. calcium oxide
D. calcium phosphate

124. Chapter 14
Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.
A. calcium sulfate
B. calcium hydroxide
C. calcium oxide
D. calcium phosphate

125. Chapter 14
Which of the following statements is true for the reaction below?
A. HF is the base. B.
C. F− is the conjugate base. D.

126. Chapter 14
Which of the following statements is true for the reaction below?
A. HF is the base. B.
C. F− is the conjugate base.
D. H2PO4- is conjugate acid

127. Chapter 14
Short Answer
Identify the conjugate acid-base pairs in the following
reaction:

128. Chapter 14
Short Answer
Identify the conjugate acid-base pairs in the following
reaction:
Answer: HClO2(aq) acid1,
NH3(aq) base2,

129. What is the pH of a 0.0010 M HNO3? A. 1.0 B. 3.0 C. 4.0 D. 5.0
Chapter 15
What is the pH of a M HNO3?
A. 1.0
B. 3.0
C. 4.0
D. 5.0

130. What is the pH of a 0.0010 M HNO3? A. 1.0 B. 3.0 C. 4.0 D. 5.0
Chapter 15
What is the pH of a M HNO3?
A. 1.0
B. 3.0
C. 4.0
D. 5.0

131. Which of the following solutions would have a pH value greater than 7?
Chapter 15
Which of the following solutions would have a pH value greater than 7?
A. [OH−] = 2.4 × 10−2 M
B. [H3O+] = 1.53 × 10−2 M
C M HCl
D. [OH−] = 4.4 × 10−9 M

132. Which of the following solutions would have a pH value greater than 7?
Chapter 15
Which of the following solutions would have a pH value greater than 7?
A. [OH−] = 2.4 × 10−2 M
B. [H3O+] = 1.53 × 10−2 M
C M HCl
D. [OH−] = 4.4 × 10−9 M

133. If the pH of a solution of the strong base NaOH
Chapter 15
If the pH of a solution of the strong base NaOH
is known, which property of the solution can be
calculated?
A. molar concentration
B. [OH−]
C. [H3O+]
D. All of the above

134. If the pH of a solution of the strong base NaOH
Chapter 15
If the pH of a solution of the strong base NaOH
is known, which property of the solution can be
calculated?
A. molar concentration
B. [OH−]
C. [H3O+]
D. All of the above

135. A neutral aqueous solution A. has a 7.0 M H3O+ concentration.
Chapter 15
A neutral aqueous solution
A. has a 7.0 M H3O+ concentration.
B. contains neither hydronium ions nor hydroxide
ions.
C. has an equal number of hydronium ions and
hydroxide ions.
D. None of the above

136. A neutral aqueous solution A. has a 7.0 M H3O+ concentration.
Chapter 15
A neutral aqueous solution
A. has a 7.0 M H3O+ concentration.
B. contains neither hydronium ions nor hydroxide
ions.
C. has an equal number of hydronium ions and
hydroxide ions.
D. None of the above

137. Chapter 15
Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.
A. calcium sulfate
B. calcium hydroxide
C. calcium oxide
D. calcium phosphate

138. Chapter 15
Identify the salt that forms when a solution of H2SO4 is titrated with a solution of Ca(OH)2.
A. calcium sulfate
B. calcium hydroxide
C. calcium oxide
D. calcium phosphate

139. The pH of a solution is 6.32. What is the pOH? A. 6.32 B. 4.8 × 10−7
Chapter 15
The pH of a solution is What is the pOH?
A. 6.32
B. 4.8 × 10−7
C. 7.68
D. 2.1 × 10−8

140. The pH of a solution is 6.32. What is the pOH? A. 6.32 B. 4.8 × 10−7
Chapter 15
The pH of a solution is What is the pOH?
A. 6.32
B. 4.8 × 10−7
C. 7.68
D. 2.1 × 10−8

141. Which of the pH levels listed below is the most acidic? A. pH = 1
Chapter 15
Which of the pH levels listed below is the most acidic?
A. pH = 1
B. pH = 5
C. pH = 9
D. pH = 13

142. Which of the pH levels listed below is the most acidic? A. pH = 1
Chapter 15
Which of the pH levels listed below is the most acidic?
A. pH = 1
B. pH = 5
C. pH = 9
D. pH = 13

143. Chapter 15
Short Answer
A solution has a pH of What is the hydronium ion concentration? Is the solution acidic or basic?

144. Chapter 15
Short Answer
A solution has a pH of What is the hydronium ion concentration? Is the solution acidic or basic?
Answer: [H3O+] = 1.8 × 10−5 M; acidic

145. Extended Response
The hydroxide ion concentration in a solution is 1.6 × 10−11 M. What are the [H3O+], the pH, and the pOH of the solution?

146. Extended Response
The hydroxide ion concentration in a solution is 1.6 × 10−11 M. What are the [H3O+], the pH, and the pOH of the solution?
Answer: [H3O+] = 6.3 × 10−4 M
pH = 3.20
pOH = 10.80

147. Chapter 17 To be effective, a collision requires
A. enough energy only.
B. favorable orientation only.
C. enough energy and a favorable orientation.
D. a reaction mechanism.

148. Chapter 17 To be effective, a collision requires
A. enough energy only.
B. favorable orientation only.
C. enough energy and a favorable orientation.
D. a reaction mechanism.

149. Chapter 17
How does the energy of the activated complex compare with the energies of the reactants and products?
A. It is lower than both the energy of the reactants and the energy of the products.
B. It is lower than the energy of the reactants but higher than the energy of the products.
C. It is higher than the energy of the reactants but lower than the energy of the products.
D. It is higher than both the energy of the reactants and the energy of the products.

150. Chapter 17
How does the energy of the activated complex compare with the energies of the reactants and products?
A. It is lower than both the energy of the reactants and the energy of the products.
B. It is lower than the energy of the reactants but higher than the energy of the products.
C. It is higher than the energy of the reactants but lower than the energy of the products.
D. It is higher than both the energy of the reactants and the energy of the products.

151. Chapter 17
If a collision between molecules is very gentle, the molecules are
A. more likely to be oriented favorably.
B. less likely to be oriented favorably.
C. likely to react.
D. likely to rebound without reacting.

152. Chapter 17
If a collision between molecules is very gentle, the molecules are
A. more likely to be oriented favorably.
B. less likely to be oriented favorably.
C. likely to react.
D. likely to rebound without reacting.

153. Chapter 17
A species that changes the rate of a reaction but is neither consumed nor changed is
A. a catalyst.
B. an activated complex.
C. an intermediate.
D. a reactant.

154. Chapter 17
A species that changes the rate of a reaction but is neither consumed nor changed is
A. a catalyst.
B. an activated complex.
C. an intermediate.
D. a reactant.

155. Chapter 17 Multiple Choice Standardized Test Preparation
6. A rate law relates
A. reaction rate and temperature.
B. reaction rate and concentration.
C. temperature and concentration.
D. energy and concentration.

156. Chapter 17 Multiple Choice 6. A rate law relates
A. reaction rate and temperature.
B. reaction rate and concentration.
C. temperature and concentration.
D. energy and concentration.

157. Chapter 17
Short Answer
10. Two molecules collide but bounce apart unchanged. What two reasons could account for their failure to react?

158. Chapter 17
Short Answer
10. Two molecules collide but bounce apart unchanged. What two reasons could account for their failure to react?
Answer: They had insufficient energy for bonds to break, or they did not collide in a favorable orientation.

159. Chapter 17
Short Answer
11. Sketch a diagram that shows how the energy changes with the progress of an endothermic reaction. Label the curve “Reactants,” “Products,” and “Activated complex.” On the same diagram, sketch a second curve to show the change caused by a catalyst.

160. Chapter 17
Short Answer
11. Sketch a diagram that shows how the energy changes with the progress of an endothermic reaction. Label the curve “Reactants,” “Products,” and “Activated complex.” On the same diagram, sketch a second curve to show the change caused by a catalyst.
Answer: The humped curve should have a final plateau that is higher than its initial plateau. The second curve should share the same plateaus as the first but should have a lower hump.